FINAL: Chemistry

Electron Configuration order

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f 

7s 7p 7d 7f

Noble gas notation

Neon = 10

1s² 2s² 2p^6 = [Ne]

Atomic Radius

• Distance from nucleus to nucleus / 2

• Decreases across a period, increases down

  • Electon Shielding: Farther = Weaker.

    • Ex: Na > Cl

Ionization Nrg

• Amt of nrg required to remove an e- from an atom

• Increases across a period, decreases down

  • Ex: Na < Cl

Electron Affinity

• Amt of nrg released when an atom gains an e-

• Increases across a period, decreases down

  • Na < Cl

Ionic Radius

• The size of an atom after gain or loss of e-

• Decreases across a period, increases down

• When it loses e- (cation) its smaller

• When it gains e- (anion) its bigger 

  • Ex: Na^+ > Cl^-

Electronegativity

• Amt of attraction an atom has towards an e- within a bond

• Increases across a period, decreases down

  • F > Cs

Group 1

Alkaline metals

Group 2

Alkaline Earth Metals

Group 3-12

Transition Metals 

Group 13

Boron

Group 14

Carbon

Group 15

Nitrogen

Group 16

Oxygen

Group 17

Halogens

Group 18

Noble Gases

Metals 

Malleable (bent easily), lustrous (shiny), good conductors of heat/electricity, lose e- 

Non-Metals 

Opposite of Metal properties: poor conductors, dull, brittle, gain e- 

Metalloids

Share both properties

Linear

b - a - b

Trigonal Planar

b - a - b

|

b

Trigonal Pyramidal

.

b - a - b

|

b

Tetrahedral

b

|

b - a - b

|

b

moving from lithium to flourine the atomic radius decreases. Explain this trend in terms of effective nuclear charge and coloumbs law. Does electron shielding play a role in this trend.

The nucleus pulls electrons more strongly and the stronger attraction the closer it pulls the electrons.

Francium is more reactive then lithium. Explain in terms of atomic radius? Does electron shielding play a role?

Francium has more nrg levels and the valence electron is farther from the nucleus.

Ionizations energies

Huge jump shows its only 1 valence electron.